US6689206B2 - Process for producing yellow iron oxide pigments - Google Patents

Process for producing yellow iron oxide pigments Download PDF

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Publication number
US6689206B2
US6689206B2 US09/945,423 US94542301A US6689206B2 US 6689206 B2 US6689206 B2 US 6689206B2 US 94542301 A US94542301 A US 94542301A US 6689206 B2 US6689206 B2 US 6689206B2
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oxidation
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rate
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US20020088374A1 (en
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Ulrich Meisen
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Lanxess Deutschland GmbH
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Bayer AG
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Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G49/00—Compounds of iron
    • C01G49/02—Oxides; Hydroxides
    • C01G49/06—Ferric oxide [Fe2O3]
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B82—NANOTECHNOLOGY
    • B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
    • B82Y30/00—Nanotechnology for materials or surface science, e.g. nanocomposites
    • C—CHEMISTRY; METALLURGY
    • C09—DYES; PAINTS; POLISHES; NATURAL RESINS; ADHESIVES; COMPOSITIONS NOT OTHERWISE PROVIDED FOR; APPLICATIONS OF MATERIALS NOT OTHERWISE PROVIDED FOR
    • C09C—TREATMENT OF INORGANIC MATERIALS, OTHER THAN FIBROUS FILLERS, TO ENHANCE THEIR PIGMENTING OR FILLING PROPERTIES ; PREPARATION OF CARBON BLACK  ; PREPARATION OF INORGANIC MATERIALS WHICH ARE NO SINGLE CHEMICAL COMPOUNDS AND WHICH ARE MAINLY USED AS PIGMENTS OR FILLERS
    • C09C1/00—Treatment of specific inorganic materials other than fibrous fillers; Preparation of carbon black
    • C09C1/22—Compounds of iron
    • C09C1/24—Oxides of iron
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2002/00—Crystal-structural characteristics
    • C01P2002/60—Compounds characterised by their crystallite size
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/60—Particles characterised by their size
    • C01P2004/64—Nanometer sized, i.e. from 1-100 nanometer
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/12—Surface area
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/60—Optical properties, e.g. expressed in CIELAB-values
    • C01P2006/62—L* (lightness axis)
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/60—Optical properties, e.g. expressed in CIELAB-values
    • C01P2006/63—Optical properties, e.g. expressed in CIELAB-values a* (red-green axis)
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/60—Optical properties, e.g. expressed in CIELAB-values
    • C01P2006/64—Optical properties, e.g. expressed in CIELAB-values b* (yellow-blue axis)

Definitions

  • the present invention relates to a process for producing yellow iron oxide pigments from iron(II) chloride and an alkaline component by the precipitation process, wherein after addition of the ⁇ -FeOOH nucleus to the preprecipitated FeCl 2 the pH is 3 to 7.
  • the production of yellow iron oxide pigments by the precipitation process has been known for a long time.
  • the typical course of this process is described, for example, in Ullmann's Encyclopedia of Industrial Chemistry, 5 th Ed., Vol. A20, p. 297 ff.
  • the raw material generally used is iron(II) sulfate obtained during the pickling of steel sheets, or iron(II) sulfate formed during the production of titanium dioxide by the sulfate process.
  • Large quantities of FeCl 2 are also obtained in the manufacture of synthetic rutile for the production of TiO 2 .
  • an object of the present invention was the conversion of iron chloride into a high-grade useful material.
  • ⁇ -FeOOH yellow iron oxide
  • ⁇ -FeOOH yellow iron oxide
  • the precipitation process DE-A 2 455 1548 or by the Penniman process (U.S. Pat. Nos. 1,368,748, 1,327,061).
  • a nucleus is first of all produced, onto which, in a further step, additional ⁇ -FeOOH is allowed to grow relatively slowly.
  • FeCl 2 is usually not isolated as crystalline material, because its solubility in water is significantly higher than that of FeSO 4 . It is therefore in many cases more highly contaminated than FeSO 4 , which is in fact purified by the crystallization step.
  • the FeCl 2 solution frequently contains organic constituents, which can greatly influence the crystallization process.
  • iron(II) chloride solutions from steel pickling and from TiO 2 production frequently contain interfering quantities of cations of higher valency (for example, Ti, Cr, Al, V, Si), these have to be removed by precipitation using an alkaline component (EP-A 0 911 370).
  • the resulting iron chloride has a pH of between 2 and 4.
  • the nucleus In order for the FeCl 2 from steel pickling to be usable, the nucleus has to be produced by the “alkali process” (U.S. Pat. No. 2,558,304). If one now proceeds with an “alkaline” yellow nucleus in accordance with the known process for pigment formation, where preprecipitated FeCl 2 is used, the addition of the nucleus to the iron(II) chloride produces a pH of 5-7, which at temperatures of above 50° C. leads to unwanted black magnetite.
  • it is an object of the present invention was to find a process whereby yellow iron oxide pigment can be produced from preprecipitated FeCl 2 and from a nucleus produced by the alkali process.
  • the invention relates to a process for producing a yellow iron oxide pigments comprising the steps of
  • the Fe concentration of the FeCl 2 is between 70 and 220 g/l
  • the Fe(III) content of the FeCl 2 is less than 8 mol % Fe(III),
  • the temperature is 20 to 45° C.
  • the rate of oxidation in the first oxidation step is 0.5 to 10 mol % Fe(III) formed per hour
  • the pH (measured in suspension at 30° C.) at which the first oxidation step is ends is between 1.5 and 3.0
  • the temperature is 55 to 85° C.
  • the pH is increased at a rate of 0.05 to 1.0 pH/h by continuous addition of an alkaline component
  • the rate of oxidation in the second oxidation step is 0.2 to 10 mol % Fe(III) formed per hour
  • the rate of circulation of the suspension during the reaction is between 1 and 15 times per hour.
  • the invention preferably relates to a process where the following parameters can be adjusted:
  • the Fe concentration of the iron component used is between 85 and 130 g/l
  • the Fe(III) content of the Fe component used is 0.1 to 2.5 mol % Fe(III),
  • the temperature in the first oxidation step is 30 to 40° C.
  • the rate of oxidation in the first oxidation step is 4 to 7 mol % Fe(III) formed per hour
  • the pH (measured in suspension at 30° C.) at which the first oxidation step is carried out is between 2.4 and 2.8
  • the temperature in the second oxidation step is 60 to 75° C.
  • the pH in the second oxidation step is increased at a rate of 0.1 to 0.8 pH/h, by continuous addition of an alkaline component
  • the rate of oxidation in the second oxidation step is 0.4 to 4 mol % Fe(III) formed per hour
  • the rate of circulation of the suspension during the reaction is 1 and 3 times per hour.
  • the process according to the invention can contain the following steps:
  • Sodium hydroxide solution is added, with intensive stirring, to an iron(II) chloride solution with an FeCl 2 content of between 50 and 450 g/l, in a quantity sufficient to establish a pH of 3 to 5.
  • other alkaline components can be used including Ca(OH) 2 , Na 2 CO 3 or ammonia.
  • the sedimentation behavior of the accumulating hydroxide slurry or carbonate slurry can be improved by the addition of a flocculation aid. Suitable flocculation aids include the known polyacrylates or other similarly acting substances. Sedimentation behavior may optionally be improved by a subsequent oxidation, resulting in the conversion of various metal cations into oxides or oxyhydroxides of higher valency, which are more easily separable.
  • the hydroxide slurry can be removed by sedimentation, filtration or separation using a separator, the selection of the suitable apparatus or of the suitable method depending on the exact experimental conditions, the flow rates and the raw materials used.
  • the concentration of the alkaline component is 3-15 equivalents per liter (based on the stoichiometry of the reaction for the nucleus formation).
  • the quantity of alkaline precipitating agent is between 120 and 350% of the stoichiometry; preferably 150 to 250% of the required stoichiometry.
  • the precipitation is carried out at temperatures between 30° C. and 60° C., preferably 34° C. to 47° C.
  • the subsequent oxidation takes place at a rate of 5 to 50 mol % Fe(III)/h, preferably 15 to 30 mol % Fe(III)/h.
  • the nucleus obtained, after examination (particle size) is used for pigment production without further isolation.
  • Batch-operated stirred-tank reactors, reactors with emitters (two-component nozzles, liquid, gas) loop reactors or bubble columns are particularly suitable for pigment formation.
  • the alkaline nucleus is pumped over a period of 10 to 120 minutes into a solution of an Fe(II) component with an Fe content of 70 to 220 g/l Fe, preferably 85 to 130 g/l Fe.
  • an Fe(II) component with an Fe content of 70 to 220 g/l Fe, preferably 85 to 130 g/l Fe.
  • excess alkaline component in the nucleus and pH of the Fe component used a pH of between 3 and 7 (measured at 30° C.) is established.
  • Preferably preprecipitated FeCl 2 having a pH of 2 to 4 is used.
  • the mixture is heated to the first oxidation temperature of 20 to 45° C., preferably 30 to 40° C.
  • Oxidation is then carried out using an oxidizing agent at a rate of 0.5 to 10 mol %/h Fe(III) formed, preferably 4 to 7 mol %/h.
  • This step is continued until all the Fe(OH) 2 formed by the mixing together of the alkaline yellow nucleus and the Fe component has been oxidized to ⁇ -FeOOH, which is the case at a pH of 1.5 to 3.0.
  • This is followed by heating to a temperature of 55° C. to 85° C., preferably 60° C. to 75° C.
  • the pH is increased at a rate of 0.05 to 1.0 pH/h, preferably 0.1 to 0.8 pH/h, by means of continuous addition of an alkaline precipitating agent.
  • an oxidizing agent is added continuously at a speed such that the rate of oxidation is between 0.2 and 10 mol %, preferably between 0.4 and 4 mol %, of Fe(III) formed per hour.
  • the pH is raised no further than pH 2.4 to 5.2, preferably pH 2.8 to 4.2, and the pH is then maintained at this value until the end of the reaction.
  • the rate of circulation throughout the entire reaction is between 1 and 15 times the final volume of the reaction.
  • Oxidizing agents which can be used, include:
  • the oxidation is concluded as soon as the Fe(II) content of the suspension is less than 1 mol %. A further oxidation to 100% conversion is of less use economically, but can definitely be achieved.
  • Suitable alkaline components include:
  • ammonia (as solution or gas)
  • Sparingly soluble compounds for example, MgCO 3
  • MgCO 3 Sparingly soluble compounds
  • iron(II) chloride may be partially replaced by iron(II) sulfate or by another economical source of Fe. But the preferred embodiment is the exclusive use of iron(II) chloride.
  • iron(III) chloride obtained during the production of TiO 2 by the chloride process to iron(II) chloride by means of metallic iron.
  • This iron(II) chloride solution can then be subjected to the purification by preprecipitation described above.
  • the yellow iron oxide pigment obtained is particularly suitable for coloring plastics or paper, or for the production of emulsion paints or other coatings and paints.
  • the pigment can be isolated from the pigment suspension by the known steps of filtration, drying and grinding.
  • the FeCl 2 solution obtained had the following properties:
  • the FeCl 2 solution obtained had the following properties:
  • the FeCl 2 solution used had the following properties:
  • the alkaline yellow nucleus obtained had the following properties:
  • the quantity of NaOH was thus 150% of the stoichiometry.
  • the solution was aerated with 100 Nl/h of air.
  • the oxidation time was 225 minutes, which corresponds to a rate of oxidation of 26.7 mol % Fe(III)/h.
  • the alkaline yellow nucleus obtained had the following properties:
  • Example 5 The procedure was as indicated in Example 5, but precipitation took place at a temperature of 44° C.
  • the oxidation time was 217 minutes, which corresponds to a rate of oxidation of 27.6 mol % Fe(III)/h.
  • the alkaline yellow nucleus obtained had the following properties:
  • Example 5 The procedure was as indicated in Example 5, but an FeCl 2 which had not been preprecipitated was used, as described in Example 3.
  • the oxidation time was 226 minutes, which corresponds to a rate of oxidation of 26.7 mol % Fe(III)/h.
  • the alkaline yellow nucleus obtained had the following properties:
  • the rate of oxidation in the first oxidation step was 5.6 mol % Fe(III) formed per hour.
  • the mixture was then heated to 60° C. and the second oxidation step was started with 36 Nl/h air.
  • the pH increased at a rate of 0.2 pH/h; the end point of the rise in pH was pH 3.4.
  • the pH was maintained constant at 3.4+/ ⁇ 0.2 by means of sodium hydroxide solution.
  • the rate of oxidation in the second oxidation step was 0.47 mol % Fe(III) formed per hour.
  • the duration of the second oxidation step was 2140 minutes.
  • the circulation performance of the stirrer based on the final volume of 22 liters, was 13.6 per hour. During the oxidation, samples were withdrawn, filtered, washed and dried and their tristimulus values determined.
  • Rate of oxidation of second oxidation step 0.42 mol % Fe(III)/h.
  • Example 8 The procedure here was as in Example 8, but the yellow nucleus from Example 4 was used. The FeCl 2 described in Example 1 was used. The differences from Example 8 are shown in the following Table. Conditions of measurement and other conditions were as described in Example 8.
  • Quantity of nucleus 2.0 mol Quantity of FeCl 2 : 18.8 mol pH prior to first oxidation: 5.5 Temperature of first oxidation: 35° C. Rate of first oxidation: 5.2 mol % Fe(III)/h pH after first oxidation: 2.2 Quantity of air in 2nd oxidation: 12 NI/h Temperature of 2nd oxidation: 75° C. Rate of 2nd oxidation: 3.6 mol % Fe(III)/h

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  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Organic Chemistry (AREA)
  • Nanotechnology (AREA)
  • Composite Materials (AREA)
  • Condensed Matter Physics & Semiconductors (AREA)
  • General Physics & Mathematics (AREA)
  • Materials Engineering (AREA)
  • Crystallography & Structural Chemistry (AREA)
  • Physics & Mathematics (AREA)
  • Inorganic Chemistry (AREA)
  • Compounds Of Iron (AREA)
  • Pigments, Carbon Blacks, Or Wood Stains (AREA)
US09/945,423 2000-09-08 2001-08-31 Process for producing yellow iron oxide pigments Expired - Fee Related US6689206B2 (en)

Applications Claiming Priority (6)

Application Number Priority Date Filing Date Title
DE10044398.2 2000-09-08
DE10044398A DE10044398A1 (de) 2000-09-08 2000-09-08 Verfahren zur Herstellung von Eisenoxidgelbpigmenten
DE10044398 2000-09-08
DE10050682A DE10050682A1 (de) 2000-09-08 2000-10-13 Verfahren zur Herstellung von Eisenoxidpigmenten
DE10050682.8 2000-10-13
DE10050682 2000-10-13

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US (1) US6689206B2 (de)
EP (1) EP1339803B1 (de)
JP (1) JP2004509043A (de)
AT (1) ATE282670T1 (de)
AU (1) AU2001293790A1 (de)
BR (1) BR0113729A (de)
CA (1) CA2421290A1 (de)
DE (3) DE10044398A1 (de)
DK (1) DK1339803T3 (de)
ES (1) ES2233692T3 (de)
WO (1) WO2002020675A1 (de)

Cited By (11)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20050282219A1 (en) * 2002-11-06 2005-12-22 Prober James M Microparticle-based methods and systems and applications thereof
US20060048828A1 (en) * 2004-09-03 2006-03-09 Ranco Incorporated Of Delaware Reversing valve with flowsplitter
US20070261604A1 (en) * 2006-05-13 2007-11-15 Carsten Rosenhahn Yellow iron oxide pigments
US20070277703A1 (en) * 2006-06-02 2007-12-06 Iop Specialists Sdn. Bhd. Iron oxide pigments from mill scale
US20080110371A1 (en) * 2006-11-09 2008-05-15 Sun Chemical Corporation Security pigments and the process of making thereof
US20080110372A1 (en) * 2006-11-09 2008-05-15 Hollman Aaron M Multi-Colored Lustrous Pearlescent Pigments and Process for Making
US20080118452A1 (en) * 2006-11-09 2008-05-22 Hollman Aaron M Cosmetic Comprising Multi-Colored Lustrous Pearlescent Pigments
US20080124575A1 (en) * 2006-11-09 2008-05-29 Hollman Aaron M Coating, Ink, or Article Comprising Multi-Colored Lustrous Pearlescent Pigments
US7399454B2 (en) 2004-04-29 2008-07-15 Metalox International, Llc Metallurgical dust reclamation process
US20090208436A1 (en) * 2006-11-09 2009-08-20 Aaron Hollman Orange pearlescent pigments
US8349067B2 (en) 2006-11-09 2013-01-08 Sun Chemical Corp. Multi-colored lustrous pearlescent pigments

Families Citing this family (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
DE10010940A1 (de) * 2000-03-06 2001-09-13 Bayer Ag Verfahren zur Herstellung von Eisenoxid und seine Verwendung
EP1512726B1 (de) * 2003-09-03 2015-10-14 LANXESS Deutschland GmbH Verfahren zur herstellung von eisenoxidgelbpigmenten mit caco3 als fällungsmittel
MX2007000357A (es) * 2004-06-27 2008-03-13 Joma Chemical As Metodo para producir nanoparticulas de oxido de hierro.
US20090185992A1 (en) * 2008-01-18 2009-07-23 Christelle Conan Process for producing iron oxide coated pearlescent pigments
CN104973623B (zh) * 2015-06-24 2016-06-01 中国大唐集团科学技术研究院有限公司华中分公司 一种利用废弃烟气脱硝催化剂制备颜料的方法
CN107265512B (zh) * 2017-06-26 2018-10-23 杭州金丰环保科技有限公司 一种全密封氧气氧化法生产氧化铁黄的方法
CN107265511B (zh) * 2017-06-26 2018-11-20 杭州金丰环保科技有限公司 一种生产氧化铁黄的方法
CN110228823B (zh) * 2019-07-03 2021-09-07 正太新材料科技有限责任公司 一种氧化铁黄及其制备方法以及氧化铁红及其制备方法

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US1368748A (en) 1920-01-05 1921-02-15 Nat Ferrite Company Process of manufacturing iron compounds and product
US2558304A (en) 1948-03-11 1951-06-26 American Cyanamid Co Production of iron oxide pigments
GB1445288A (en) 1973-11-21 1976-08-11 Tdk Electronics Co Ltd Process for producing goethite
US4459276A (en) * 1981-09-17 1984-07-10 Agency Of Industrial Science & Technology Yellow iron oxide pigment and method for manufacture thereof
US5451253A (en) 1993-04-02 1995-09-19 Basf Aktiengesellschaft Preparation of transparent yellow iron oxide pigments
US5879441A (en) 1994-09-30 1999-03-09 Bayer Ag Very highly transparent yellow iron oxide pigments, a process for their production and their use
US5916360A (en) * 1996-12-19 1999-06-29 Bayer Ag Process for the preparation of iron oxide yellow pigments and the use thereof
US6027559A (en) * 1997-06-23 2000-02-22 Toda Kogyo Corporation Yellow iron oxide hydroxide particles and process for producing the same
US6042642A (en) 1997-10-20 2000-03-28 Bayer Ag Iron oxide yellow pigments, a method of producing iron oxide yellow pigments and the use thereof
US6179908B1 (en) 1997-10-20 2001-01-30 Bayer Ag Iron oxide red pigments, process for the production of iron oxide red pigments and use thereof

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DE3922106A1 (de) 1989-07-05 1991-01-17 Bayer Ag Synthetisches grobteiliges eisenoxid, verfahren zu seiner herstellung sowie dessen verwendung

Patent Citations (11)

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US1327061A (en) 1917-06-20 1920-01-06 West Coast Kalsomine Company Process of manufacturing iron compounds
US1368748A (en) 1920-01-05 1921-02-15 Nat Ferrite Company Process of manufacturing iron compounds and product
US2558304A (en) 1948-03-11 1951-06-26 American Cyanamid Co Production of iron oxide pigments
GB1445288A (en) 1973-11-21 1976-08-11 Tdk Electronics Co Ltd Process for producing goethite
US4459276A (en) * 1981-09-17 1984-07-10 Agency Of Industrial Science & Technology Yellow iron oxide pigment and method for manufacture thereof
US5451253A (en) 1993-04-02 1995-09-19 Basf Aktiengesellschaft Preparation of transparent yellow iron oxide pigments
US5879441A (en) 1994-09-30 1999-03-09 Bayer Ag Very highly transparent yellow iron oxide pigments, a process for their production and their use
US5916360A (en) * 1996-12-19 1999-06-29 Bayer Ag Process for the preparation of iron oxide yellow pigments and the use thereof
US6027559A (en) * 1997-06-23 2000-02-22 Toda Kogyo Corporation Yellow iron oxide hydroxide particles and process for producing the same
US6042642A (en) 1997-10-20 2000-03-28 Bayer Ag Iron oxide yellow pigments, a method of producing iron oxide yellow pigments and the use thereof
US6179908B1 (en) 1997-10-20 2001-01-30 Bayer Ag Iron oxide red pigments, process for the production of iron oxide red pigments and use thereof

Cited By (19)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20050282219A1 (en) * 2002-11-06 2005-12-22 Prober James M Microparticle-based methods and systems and applications thereof
US7399454B2 (en) 2004-04-29 2008-07-15 Metalox International, Llc Metallurgical dust reclamation process
US20060048828A1 (en) * 2004-09-03 2006-03-09 Ranco Incorporated Of Delaware Reversing valve with flowsplitter
US20070261604A1 (en) * 2006-05-13 2007-11-15 Carsten Rosenhahn Yellow iron oxide pigments
US20070277703A1 (en) * 2006-06-02 2007-12-06 Iop Specialists Sdn. Bhd. Iron oxide pigments from mill scale
US7347893B2 (en) * 2006-06-02 2008-03-25 Iop Specialists Sdn. Bhd. Iron oxide pigments from mill scale
US20080124575A1 (en) * 2006-11-09 2008-05-29 Hollman Aaron M Coating, Ink, or Article Comprising Multi-Colored Lustrous Pearlescent Pigments
US20080118452A1 (en) * 2006-11-09 2008-05-22 Hollman Aaron M Cosmetic Comprising Multi-Colored Lustrous Pearlescent Pigments
US20080110372A1 (en) * 2006-11-09 2008-05-15 Hollman Aaron M Multi-Colored Lustrous Pearlescent Pigments and Process for Making
US20080110371A1 (en) * 2006-11-09 2008-05-15 Sun Chemical Corporation Security pigments and the process of making thereof
US20090038514A2 (en) * 2006-11-09 2009-02-12 Sun Chemical Corporation Multi-Colored Lustrous Pearlescent Pigments
US20090208436A1 (en) * 2006-11-09 2009-08-20 Aaron Hollman Orange pearlescent pigments
US7850775B2 (en) 2006-11-09 2010-12-14 Sun Chemical Corporation Multi-colored lustrous pearlescent pigments
US8211224B2 (en) 2006-11-09 2012-07-03 Sun Chemical Corp. Multi-colored lustrous pearlescent pigments and process for making
US8221536B2 (en) 2006-11-09 2012-07-17 Sun Chemical Corp. Cosmetic comprising multi-colored lustrous pearlescent pigments
US8323396B2 (en) 2006-11-09 2012-12-04 Sun Chemical Corp. Orange pearlescent pigments
US8349067B2 (en) 2006-11-09 2013-01-08 Sun Chemical Corp. Multi-colored lustrous pearlescent pigments
US8486189B2 (en) 2006-11-09 2013-07-16 Sun Chemical Corporation Cosmetic comprising multi-colored lustrous pearlescent pigments
US8906154B2 (en) 2006-11-09 2014-12-09 Sun Chemical Corporation Coating, ink, or article comprising multi-colored lustrous pearlescent pigments

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Publication number Publication date
ES2233692T3 (es) 2005-06-16
DE50104567D1 (de) 2004-12-23
US20020088374A1 (en) 2002-07-11
WO2002020675A1 (de) 2002-03-14
EP1339803A1 (de) 2003-09-03
EP1339803B1 (de) 2004-11-17
CA2421290A1 (en) 2003-03-05
AU2001293790A1 (en) 2002-03-22
JP2004509043A (ja) 2004-03-25
BR0113729A (pt) 2003-07-22
DE10050682A1 (de) 2002-04-18
DK1339803T3 (da) 2005-01-24
DE10044398A1 (de) 2002-03-21
ATE282670T1 (de) 2004-12-15

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